For the reaction `2NO(g)+O_(2)(g)to2NO_(2)g` Calculate `DeltaG` at 700K when enthalpy and entropy changes are `-113.0kJ" "mol^(-1) and `-145J" "K^(-1)mol^(-1)` respectively.

For the reaction `2NO(g)+O_(2)(g)to2NO_(2)g` Calculate `DeltaG` at 700

1.	For the reaction `2NO(g)+O_(2)(g)to2NO_(2)g` Calculate `DeltaG` at 700K when enthalpy and entropy changes are `-113.0kJ" "mol^(-1) and `-145J" "K^(-1)mol^(-1)` respectively.
Answer» We know that `DeltaG=DeltaH-TDeltaS` Given, `DeltaH=-113kJ" "mol^(-1)` `=-113000J" "mol^(-1)` `DeltaS=-145J" "K^(-1)" "mol^(-1)` `T=700K` Substituting these values in the above equation, we get `DeltaG=-113000-700xx(-145)` `=-11500J" "mol^(-1)` `=-11.5kJ" "mol^(-1)`

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For the reaction `2NO(g)+O_(2)(g)to2NO_(2)g` Calculate `DeltaG` at 700K when enthalpy and entropy changes are `-113.0kJ" "mol^(-1) and `-145J" "K^(-1)mol^(-1)` respectively.

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